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  • A gaseous reaction, <img alt="\mathrm{A_2(g)+B_2(g) \rightarrow C_2(g)}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7BA_2%28g%29&plus;B_2%28g%29%20%5Crightarrow%20C_2%28g%29

A gaseous reaction, \mathrm{A_2(g)+B_2(g) \rightarrow C_2(g)} , shows increase in pressure from 50 $\mathrm{mm}$ to \mathrm{60 \mathrm{~mm}} in 10 minutes. The rate of disappearance of \mathrm{\mathrm{A}_2}  is

Option: 1

\mathrm{4 mm ~min^{-1} }


Option: 2

\mathrm{8 mm~ min^{-1} }


Option: 3

\mathrm{1 mm~ min^{-1} }


Option: 4

\mathrm{2 mm ~min^{-1}}


Answers (1)

best_answer

Given initial pressure 50 mm and final pressure 60 mm.

 

\mathrm{A_2(g)+B_2(g)\rightarrow C_2(g)}

t = 0

50 mm

           

t = 10 min

(50 – x) mm

x

x

\text { At } \mathrm{t}=10 \mathrm{~min} \text {, Pressure }=50-\mathrm{x}+\mathrm{x}+\mathrm{x} =60 \mathrm{~mm} \text { (given) }

x =10 \mathrm{~mm}

Now, the rate of disappearance of A_2 is \frac{d[A]}{d t}=\frac{10 \mathrm{~mm}}{10 \mathrm{~min}}=1 \mathrm{~mm} \mathrm{~min}^{-1}

Posted by

Rishabh

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